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Chemistry: Electron Arrangements and Periodicity Study Guide
1.
Visible light, X rays, infrared radiation, and radio waves all have the same_________________________.
2.
The distance between two successive peaks/crests on adjacent waves is its__________________________.
3.
A quantum of electromagnetic energy is called a(n)___________________________________.
4.
For an electron in an atom to change from the ground state to an excited state, What must happen to the energy?
5.
If electrons in an atom have the lowest possible energies, the atom is in the___________________state.
6.
The quantum number that indicates the position of an orbital about the three axes in space is
the_________________________________________________ number
7.
The main energy levels of an atom are indicated by the_________________________________number.
8.
The spin quantum number of an electron can be thought of as describing the _______________of electron spin.
9.
The set of orbitals that are dumbbell shaped and directed along the x, y, and z axes are called_________________
orbitals.
10.
A spherical electron cloud surrounding an atomic nucleus would best represent the ________________orbital.
11.
The p orbitals are shaped like____________________________.
12.
How many electrons can occupy the s orbitals at each energy level?__________________________________
13.
How many electrons are needed to completely fill the fourth energy level?___________________________.
14.
The main energy level that can hold only two electrons is the________________________________.
15.
The statement that an electron occupies the lowest available energy orbital is_______________________principle.
16.
"Orbitals of equal energy are each occupied by one electron before any is occupied by a second electron, and all
electrons in singly occupied orbitals must have the same spin" is a statement of____________________________.
17.
Two electrons in the 1s orbital must have different spin quantum numbers to satisfy the
____________________principle.
18.
The Aufbau principle states that an electron____________________________________________________
_____________________________________________________________________________________.
19.
The Pauli exclusion principle states that no two electrons in the same atom can________________________
____________________________________________________________________________________.
20.
What is the electron configuration for carbon, atomic number 6?
______________________________________________________________________________________________
21.
The electron notation for magnesium (atomic number 12) is
_______________________________________________________________________________________________
22.
If an element has an octet of electrons in its highest main energy level, there are ____ electrons in this level.
23.
An element with 8 electrons in its highest main energy level is a(n)_________________________________.
24.
The periodic law states that the physical and chemical properties of elements are periodic functions of their
atomic_________________
25.
The principle that states that the physical and chemical properties of the elements are periodic functions of their
atomic numbers is_________________________
26.
Elements in a group or column in the periodic table can be expected to have similar______________________.
27.
The element that has the greatest electronegativity is_____________________________.
28.
In a row in the periodic table, as the atomic number increases, the atomic radius generally_________________.
29.
The number of valence electrons in Group 1 elements is______________________________.
30.
In Group 2 elements, the valence electrons are in sublevel______________________.
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31. Which element has the following electron configuration: [Ar] 4s2 3d10 4p5?
32. Write the noble-gas electron configuration for silicon.
33. Draw the orbital diagram for phosphorus.
34. Draw the orbital diagram for argon.
35. What element's orbital diagram is shown in the figure below?
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